If you increase the atmospheric pressure, the pressure will also increase. This is because atmospheric pressure is the pressure exerted by the weight of air above a certain point, so increasing the amount of air causes an increase in pressure.
Increasing the temperature the number of particles remain constant and the pressure increase.
The initial total pressure is 1.0 ATM + 2.0 ATM = 3.0 ATM. Therefore, 6.0 ATM - 3.0 ATM = 3.0 ATM of helium was added to the tank. Hence, the partial pressure of helium in the tank is 3.0 ATM.
To find the total pressure inside the container, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of the individual gases. Therefore, the total pressure would be 2.0 ATM (Ne) + 1.5 ATM (He) + 2.5 ATM (N2) = 6.0 ATM. Thus, the pressure inside the container is 6.0 ATM.
To find the pressure of gas B, you can use Dalton's Law of Partial Pressures, which states that the total pressure is the sum of the partial pressures of individual gases. Given that the total pressure is 1.20 ATM and the partial pressure of gas A is 0.75 ATM, you can calculate the pressure of gas B as follows: Pressure of gas B = Total pressure - Pressure of gas A = 1.20 ATM - 0.75 ATM = 0.45 ATM. Thus, the pressure of gas B is 0.45 ATM.
If you put pressure on ice it will melt.
A. An increase in pressure from 2 ATM to 3 ATM will result in a decrease in volume of gas. B. An increase in pressure from 3 ATM to 4 ATM will result in a decrease in volume of gas. C. A decrease in pressure from 4 ATM to 1 ATM will result in an increase in volume of gas. D. An increase in pressure from 1 ATM to 3 ATM will result in a decrease in volume of gas.
As pressure increases from 0.8 ATM to 1.2 ATM, the boiling point of water also increases. Therefore, at 100°C and 0.8 ATM, water would boil, but at 1.2 ATM, the water would need to be heated to a higher temperature to reach the new boiling point under the increased pressure.
At 212 oF, water boils at 1 atm of pressure.
The pressure will increase.
Increasing the temperature the number of particles remain constant and the pressure increase.
The pressure will increase.
At -50°C and 1 atm, the substance is in the solid phase. With an increase in pressure to 3 atm, the phase transition will occur from the solid phase to the liquid phase.
1.54 atm
1.54 atm
At 2.5 ATM of pressure, water would boil at a higher temperature than 100°C. The boiling point of water increases as pressure increases. For every increase of 1 ATM in pressure, the boiling point of water increases by 10°C. Therefore, at 2.5 ATM, water would boil at approximately 125°C.
The total pressure of the mixed gases will be 5 ATM. The partial pressure of each gas will remain the same as their individual pressures before mixing, so the partial pressure for the gas originally at 2 ATM will remain at 2 ATM, and the gas originally at 3 ATM will remain at 3 ATM.
The solubility of oxygen in blood at 2 ATM (double atmospheric pressure) is greater than at atmospheric pressure because gases are more soluble in liquids at higher pressures. This means that the blood can carry more oxygen when exposed to higher pressures, such as when diving.